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Chapter 4
Aqueous solutions
Types of reactions
mixture
homogeneous heterogeneous
one phaseTab water
two phasesoil/water
milk
solution
solvent Solute(s)more abundant component of
mixturewater in tab
water
Less abundant or other component(s) of mixturesalts in tab water
Water always solvent even in 98% H2SO4
solutes
ElectrolytesNon-
electrolytes
Solute undergoes Dissociation
strong weakcomplete
dissociationpartial
dissociationNaCl / H2OHCl / H2O
HAc / H2O
Sugar / H2O
)()()(2
aqaqOH
s ClNaNaCl )()()(2
aqaqOH
l AcHHAc
Hydration of Solid Solute
At edges, fewer oppositely charged ions around– H2O can come in; Ion-dipole forces; Remove ion
New ion at surface– Process continues until all ions in solution
Hydration of ions – Completely surrounded by solvent
4
Molecular Compounds In Water When molecules dissolve in water
– Solute particles are surrounded by water– Molecules are not dissociated
5
Electrical conductivityof electrolyte solutions
Ionic compounds
Strong acids and bases
Ex. NaBr, KNO3, HClO4, HCl, KOH
Weak acids and bases
Ex. Acetic acid (HC2H3O2), ammonia (NH3)
Ex. Sugar, alcohol
Learning Check
Write the equations that illustrate the dissociation of the following salts:
Na3PO4(aq) →
Al2(SO4)3(aq) →
CaCl2(aq) →
Ca(MnO4)2(aq) →7
3 Na+(aq) + PO43(aq)
Ca2+(aq) + 2 Cl(aq)
Solubility Maximum amount of a substance that can be
dissolved in a given amount of solvent at a given temperature.
Usually g/100 mL.
solvent g 100
solution saturated make toneeded gSolubility
solute
Saturated solution: Solution in which no more solute can be dissolved at a given temperatureUnsaturated solution: Solution containing less solute
than max. amount; Able to dissolve more solute
Solubilities of Some Common Substances
9
Substance FormulaSolubility
(g/100 g water)
Sodium chloride NaCl 35.7 at 0°C39.1 at 100°C
Sodium hydroxide
NaOH 42 at 0°C347 at 100°C
Calcium carbonate
CaCO3 0.0015 at 25°C
“Like dissolves Like” Ethanol (C2H5OH) dissolves in water:
polar ↔ polar
Glucose (C6H12O6) and sucrose (C12H22O11)
dissolve in water: polar ↔ polar
Oil doesn’t dissolve in water: nonpolar ↔ polar Oil dissolves in benzene: nonpolar ↔ nonpolar
Salts are polar.
soluble insolubleNaCl AgCl
Water unable to separate Ag+ from
Cl-
Interaction very strong
Relative Concentration
Dilute solution– Small solute to solvent ratio
Ex. Eyedrops
Concentrated solution– Large solute to solvent
ratio
Ex. Pickle brine
Dilute solution contains less solute per unit volume than more concentrated solution
12
Solute-to-solvent ratio
quantitatively
abbreviated M 1 M = 1 mol solute / 1 liter solution
Molarity
LV
nM
solution
solute
/
molmolg
g
M
mn
NaOH
NaOHNaOH 288.0
/0.40
5.11
ML
mol
L
mol
LV
nM
solution
NaOHNaOH 192.0192.0
50.1
288.0
/
Preparing Solution of Known Molarity
a b c d e
a) Weigh solid and transfer to volumetric flask
b) Add part of the water
c) Dissolve solute completely
d) Add water to reach etched line
e) Stopper flask and invert to mix thoroughly 14
Concentration of each type of ions in 0.50 M Co(NO3)2(aq)?
)(3)(2
)(23 2)( aqaqaq NOCoNOCo 1 mol 1 mol 2 mol
In 1.00 L 0.50 mol 0.50 mol 1.00 mol
Molarity 0.50 M 0.50 M 1.00 M
Concentration of each type of ions in 0.50 M Fe(ClO4)3(aq)?
)(4)(3
)(34 3)( aqaqaq ClOFeClOFe
Molarity 0.50 M 0.50 M 1.50 M
Moles of Cl- 1.75 L of 1.0×10-3 M ZnCl2(aq)?
molLL
moln
LMn
LVMnLV
nM
ZnCl
ZnCl
solutionZnClZnClsolution
ZnClZnCl
33
3
1075.175.1100.1
75.1100.1
//
2
2
22
2
2
)()(2
)(2 2 aqaqaq ClZnZnCl
1 2
1.75×10-3 mol ? moln
moln
Cl
Cl
3
3
105.3
1075.12
mol
gmolMnm
ClClCl45.351075.12 3
NaCl
NaClsolution
solution
NaClNaCl M
nV
LV
nM
/
molmolg
g
M
mn
NaCl
NaClNaCl
53
107.1/44.58
100.1
mLLLmol
mol
M
nV
NaCl
NaClsolution 12.0102.1
/14.0
107.1 45
Practice How many grams of HCl would be required to make
50.0 mL of a 2.7 M solution?
What would the concentration be if you used 27g of CaCl2 to make 500. mL of solution? What is the concentration of each ion?
Describe how to make 1.00 L of a 0.200 M K2CrO4 solution.
Describe how to make 250. mL of an 2.0 M copper (II) sulfate dihydrate solution.
Calculate the concentration of a solution made by dissolving 45.6 g of Fe2(SO4)3 to 475 mL. What is the concentration of each ion?
Describe how to make 1.00 L of a 0.200 M K2CrO4 solution.
molLMn
LVMnLV
nM
CrOK
solutionCrOKCrOKsolution
CrOKCrOK
200.000.1200.0
//
42
4242
42
42
gmolgmolMnm CrOKCrOKCrOK 8.58/20.294200.0424242
No solid K2CrO4 available in the
lab .But 2.00 M K2CrO4 solution is
available .
molLMn
LVMnLV
nM
CrOK
solutionCrOKCrOKsolution
CrOKCrOK
200.000.1200.0
//
42
4242
42
42
Dilution
2211
42424242
4242
VMVM
VMVM
VMn
nn
dilutionafterCrOKCrOKdilutionbeforeCrOKCrOK
dilutionafterCrOKdilutionbeforeCrOK
LM
LMV
LMVM
VMVM
100.000.2
00.1200.0
00.1200.000.2
1
1
2211
Prepare 150 mL of 0.100 M H2SO4 from 16.0 M solution.
mLM
mLMV
mLMVM
VMVM
938.00.16
150100.0
150100.00.16
1
1
2211
What volume of a 1.7 M solution is needed to make 250 mL of a 0.50 M solution?
18.5 mL of 2.3 M HCl is added to 250 mL of water. What is the concentration of the solution?
You have a 4.0 M stock solution. Describe how to make 1.0 L of a 0.75 M solution.
Types of Chemical Reactions
Metathesis Reduction-
OxidationDouble
Replacement
precipitation reaction
Acid-Base Reaction
precipitateFormation of a
weak electrolyte
a solid is formed from
solution
Electron transfer
Formation of a gas
AB + CD AD + CB
Precipitation reactions
Molecular equation
A reaction takes place if it has a net ionic equation
Ionic equation
)(4)(3)()(3)(2
)(2
4)( 2222 saqaqaqaqaqaq BaCrONOKNOBaCrOK
Net ionic equation: describes what really happens.
)(4)(2
4)(2
saqaq BaCrOCrOBa
Spectator ions: )(3)( 2, aqaq NOK
Solubility Rules1 All nitrates and acetates are soluble
2 Salts of alkali metals ions and NH4+ ions are soluble.
3 Chlorides, bromides and iodides (salts of Cl-, Br- and I-) are soluble except those of Ag+, Pb2+, and Hg2
2+.
4 Most sulfates are soluble, except those of Pb2+, Ba2+, Hg2+, and Ca2+.
5 Most hydroxides are slightly soluble (insoluble) except those of alkali metals (Ba(OH)2, Sr(OH)2 and Ca(OH)2 are marginally soluble).
6 Sulfides (S2-), carbonates (CO32-), chromates (CrO4
2-) and phosphates (PO4
3-), are insoluble except those of alkali metals and NH4
+.
Does the following mixing process involve a chemical reaction?
??)()(3 aqaq KClAgNO
3)()(3 KNOAgClKClAgNO aqaq
)(3)()()(3 aqsaqaq KNOAgClKClAgNO
)()()( saqaq AgClClAg
Precipitation reactions
NaOH(aq) + FeCl3(aq) ® ??
NaOH(aq) + FeCl3(aq) ® NaCl + Fe(OH)3
NaOH(aq) + FeCl3(aq) ® NaCl(aq) + Fe(OH)3(s)
Na+(aq)+OH-
(aq) + Fe3+ (aq) + Cl-(aq) ® Na+ (aq) +
Cl- (aq) + Fe(OH)3(s)
OH-(aq) + Fe3+
(aq) ® Fe(OH)3(s)
Precipitation reactions
BaCl2(aq) + KNO3(aq) ® ??
BaCl2(aq) + KNO3(aq) ® KCl + Ba(NO3)2
BaCl2(aq) + KNO3(aq) ® KCl(aq) + Ba(NO3)2(aq)
Ba2+(aq)+2 Cl-(aq) + K+
(aq) + NO3-(aq) ® K+ (aq) +
Cl- (aq) + Ba2+(aq)+ 2 NO3
-(aq)
No net ionic equation
No reaction
Practice iron (III) sulfate and potassium sulfide
Lead (II) nitrate and sulfuric acid.
solutions of NaOH and NiCl2 are mixed.
)(3)()()(3 aqsaqaq NaNOAgClNaClAgNO
molLMVMn AgNOAgNOAgNO 150.050.1100.0333
1 1
0.15 mol ? molnNaCl 150.0
gmol
gmol
Mnm NaClNaClNaCl
77.844.58150.0
1.25 L of 0.0500 M Pb(NO3)2 mixed with 2.0 L of 0.0250 M Na2SO4. Calculate the mass of
precipitate.??)( )(42)(23 aqaq SONaNOPb
)(3)(4)(42)(23 2)( aqsaqaq NaNOPbSOSONaNOPb
molLMVMn
molLMVMn
SONaSONaSONa
NOPbNOPbNOPb
0500.000.20250.0
0625.025.10500.0
424242
333 2)(2)(2)(
1 1
0.0625 mol ?
molnPbSO 0625.04
1 1
0.0500 mol ?
gMmm
molnPbSO
2.15
0500.04
Stoichiometry of Precipitation What mass of solid is formed when 100.00 mL
of 0.100 M Barium chloride is mixed with 100.00 mL of 0.100 M sodium hydroxide?
What volume of 0.204 M HCl is needed to precipitate the silver from 50.0 ml of 0.0500 M silver nitrate solution ?
25 mL 0.67 M of H2SO4 is added to 35 mL of 0.40 M CaCl2 . What mass CaSO4 Is formed?
Arrhenius Acid Substance that reacts with water to produce the
hydronium ion, H3O+
Acid + H2O Anion + H3O+
HA + H2O A– + H3O+
HC2H3O2(aq) + H2O H3O+(aq) + C2H3O2
−(aq)
HCl(g) + H2O Cl–(aq) + H3O+(aq)
Bronsted-Lowry Acid: H+ donor
Arrhenius Bases Substance that reacts with water to give OH–.
a. Metal Hydroxides
NaOH(s) Na+(aq) + OH–
(aq)
Mg(OH)2(s) Mg2+(aq) + 2OH–
(aq)
b. Basic Anhydrides
CaO(s) + H2O Ca(OH)2(aq)
Ca(OH)2(aq) Ca2+(aq) + 2OH–
(aq)
c. Molecular bases: NH3(aq)+H2O NH4
+(aq)+ OH-
(aq)
Bronsted Base: H+ acceptor
Acid-Base Reactions
??)()( aqaq NaOHHCl
)(2)()()( laqaqaq OHNaClNaOHHCl
Ionic equation
)(2)()()()()()( laqaqaqaqaqaq OHClNaOHNaClH
Weak electrolyte: H2O + H2O H3O+(aq)
+ OH-(aq)
Net ionic equation: )(2)()( laqaq OHOHH
Any strong acid + strong base
??)()(232 aqaq NaOHOHHC
)(2)(232)()(232 laqaqaq OHOHNaCNaOHOHHC
Formation of Weak electrolyte:
HAc + H2O H3O+(aq)+ Ac-
(aq)
Acid - Base Reactions are often called neutralization reaction Because the acid neutralizes the base.
Volume of 0.100 M HCl needed to neutralize 25.0 mL of 0.350 M NaOH ?
)(2)()()( laqaqaq OHNaClNaOHHCl
molLMVMn NaOHNaOHNaOH31075.80250.0350.0
1 1
? 8.75×10-3
molnHCl31075.8
L
Lmol
mol
M
nVVMn 2
3
1075.8100.0
1075.8
28.0 mL of 0.250 M HNO3 mixed with 53.0 mL of 0.320 M KOH;
1)Amount of water formed2)Concentrations of H+ and OH- at the end of rct
)(2)(3)()(3 laqaqaq OHKNOKOHHNO
mmolmLL
molVMn
mmolmLL
molVMn
KOHKOHKOH
HNOHNOHNO
0.170.53320.0
0.70.28250.0333
1 1
7.0 mmol ?
mmoln OH 0.72
1 1
17.0 mmol ? mmoln OH 172
HNO3 is Limiting reactant: reacts completely
1)No HNO3 left
2)HNO3 → H+ + NO3-
3)No H+ at the end of reaction
MmLV
nM
solution
HH
05328
0
How much remains from KOH?
1)KOH → K+ + OH-
10 → 10 mmol
mmolnnn
nnn
reactedHNOinitiallyKOHremainingKOH
reactedKOHinitiallyKOHremainingKOH
1070.173
MmL
mmol
mL
mmol
V
nM
solution
OHOH
123.081
10
5328
10
Volumetric analysis: TitrationControlled addition of 1 reactant to another until rxn is complete.
Acid-Base Titration: Very common type of titrationEx. Analysis of citric acid in orange juice by neutralization
with NaOH
An indicator is needed: organic substance that changes color according to solution acidity
Where the indicator changes color is the endpoint.
Endpoint must be very close to the equivalence point.Acid (Base) added equivalent to base (acid) present
PhenolphthaleinAcidic Basic
baseacid ntoequivalentn
Standardization of NaOH solution• Know the exact concentration!• Its weight is inaccurate .
• NaOH is hygroscopic and it absorbs CO2.
• Cannot be used to prepare solutions with exactly known M.
• Not a primary standard.• KHP is a primary standard: high purity, no weighing
problems, Potassium hydrogen phthalate: KHC8H4O4.
Monoprotic!41.2 mL of NaOH solution is needed to react exactly with 1.300 g of KHP
(M=204.22 g/mol). MNaOH=?
ML
molg
g
VMwt
mM
Mwt
mVM
nn
NaOHKHP
KHPNaOH
KHP
KHPNaOHNaOH
KHPNaOH
1546.004120.022.204
300.1
%82.56%1003518.0
1999.0%100%
1999.012.12201059.01546.0
g
g
m
macid
gmol
gL
L
molm
MwtVMm
Mwt
mVM
nn
sample
acid
acid
acidNaOHNaOHacid
acid
acidNaOHNaOH
acidNaOH
practice 75 mL of 0.25M HCl is mixed with 225 mL of
0.055 M Ba(OH)2 . What is the
concentration of the excess H+ or OH- ?
A 50.00 mL sample of aqueous Ca(OH)2 requires 34.66 mL of 0.0980 M Nitric acid for neutralization. What is [Ca(OH)2 ]?
32 2
1)( HNOOHCa nn
wheneEquivalenc